Hund's Rule means the two electrons, when paired, must be of opposite spin. The first two arrows don't have that, that is one problem. The spacing isn't what you intended, I think, so I don't know about the others. A second is 3d fills (in most cases) before 4s. Those two are all I see.

For 4s, the box has two arrows going up. For 3d, there were five boxes. The first three boxes had two arrows are up and down (correctly) in each box. The fourth box has an arrow going up. And the, fifth box is empty.

So, is this orbital diagram has a problem in aufbau principle or Pauli exclusion principle as well? What do you think?

OK. Now that you've described it a little better, this is how I would go.
The << in 4s can't be because of the Pauli Exclusion Principle (No two electrons can have the same 4 quantum numbers).
The 3d should fill before the 4s; that's the Aufbau Principle (electrons fill the lower energy levels before filling the higher energy levels.)
The 3d electrons have an empty orbital BUT some electrons in the 3d orbitals are already paired and that can't be (because Hund's rule of maximum multiplicity says that electrons don't pair until all of the orbitals have at least one electron in them.)
Note: I may not have stated the rules EXACTLY the way they are in your text or notes BUT your text may have chosen different words to say the same thing.